CHE116_Lecture6_2011

CHE116_Lecture6_2011 - Chemistry Chemistry116 Lecture6...

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hemistry 116 Chemistry 116 Lecture 6 pics sing Equilibrium Constants Topics: Using Equilibrium Constants Chapter 15.4 15.6
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The Concept of Equilibrium Chemical equilibrium occurs when a reaction and its reverse reaction proceed at the same rate. ey concept is N O ( 2 NO ( Key concept is that this action is 2 4 ( g ) 2 ( g ) reaction is reversible . clear brown
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he Equilibrium Constant The Equilibrium Constant e tio of the rate constants is a constant The ratio of the rate constants is a constant at that temperature, and the expression becomes: K q = k f [NO 2 ] 2 = eq k r [N 2 O 4 ] This is known as the equilibrium constant .
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The Equilibrium Constant Consider the generalized reaction: e equilibrium expression for this reaction aA + b Bc C + dD The equilibrium expression for this reaction (from the law of mass action ) would be: K c = [C] c [D] d ] a ] b [A] [B] The equilibrium constant depends only on the stoichiometry of the reaction, not the mechanism!
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What Does the Value of K Mean? If K >>1 , the reaction is product favored ; product predominates at equilibrium. •I f K <<1 , the reaction is actant vored reactant ; reactant predominates equilibrium at equilibrium.
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Heterogeneous Equilibria The equilibrium examples we have talked about so far are based on homogeneous equilibria. Homogeneous equilibrium means that all of the reactants and products are in the same physical state or phase. Heterogeneous equilibrium considers the equilibrium between components in different q p phases ( e.g. a solid placed in a liquid).
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Heterogeneous Equilibria The concentrations of pure solids and liquids re constant. are constant. Solid and liquid concentrations can be obtained y multiplying the density of the substance by by multiplying the density of the substance by its molar mass.
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CHE116_Lecture6_2011 - Chemistry Chemistry116 Lecture6...

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